Acid Names vs. Formulas
HI
Hydroiodic Acid
A pH in this range would indicate a basic or alkaline solution.
pH>7
If you already know the pOH of a solution, you can find the pH by doing this.
Subtracting the pOH from 14
0.0500 mol of potassium hydroxide are present in 2.50L of water. This is the pH of the solution.
pH of 12.3
A species that is a proton acceptor.
Bronsted-Lowry Base
The formula for Carbonic Acid
H2CO3
The [H+] concentration of a solution with a pH of 2.2
6.3x10-3M
The [OH-] concentration of a solution with a pOH of 3.2
6.3x10-4 M
3.2mL of concentrated 12M hydrochloric acid is diluted down to 5.0L to get this pH.
pH of 2.1
A polyprotic acid that can produce or donate two protons or H+ ions.
A diprotic acid.
HBrO
Hypobromous acid
The pH of a solution with an [H+] concentration of 1.3x10-9
pH=8.9
The pOH of a solution with an [OH-] concentration of 3.4x10-7
pOH of 6.5
13mg of citric acid is dissolved into 500.mL of water. This would be the pH of the solution.
2min
pH of 3.4
I can create one of these by combining a solution of weak acid, like phosphoric acid with it's conjugate base (usually in salt form e.g. sodium phosphate) in order to resist drastic changes in pH.
A buffer
A triprotic organic acid involving 7 oxygens.
C6H8O7
or Citric Acid
The pH of a solution with an [OH-] concentration of 7.6x10-5
The pOH of a solution with an [H+] concentration of 5.6x10-7
pOH of 7.7
The pH after 1.32mL of of concentrated 18M sulfuric acid is diluted to 3.0L.
pH of 1.8
Defined as the substance that is present after a Bronsted-Lowery Base accepts a proton or protons.
A conjugate Acid
The formula for an organic acid that, when paired with a salt like sodium acetate, would make an excellent buffer.
CH3COOH
or HC2H3O2
The pH of Sulfuric acid that is diluted down to a concentration of 1.1x10-3 M
pH = 2.7
The pOH of Hydrochloric acid that is diluted down to a concentration of 1.1x10-3 M
pOH of 11
This is the concentration of a 13.0mL phosphoric acid analyte titrated with 0.50M 15.43mL of barium hydroxide.
2min
0.40M H3PO4
This kind of acid may have a lower Ka or acid dissociation constant.
A weak acid.